Search found 97 matches
- Sun Mar 08, 2020 11:38 pm
- Forum: Zero Order Reactions
- Topic: Not used Half life
- Replies: 8
- Views: 907
Re: Not used Half life
The half-life for a first order reaction is used because it remains constant for a substance and is independent of reactant concentration.
- Sun Mar 08, 2020 11:36 pm
- Forum: Zero Order Reactions
- Topic: examples of zero order reactions?
- Replies: 6
- Views: 473
Re: examples of zero order reactions?
A zero order reaction would be an enzymatic reaction in which the enzyme is saturated so the reaction rate does not increase even if the concentration of the reactants increases.
- Sun Mar 08, 2020 11:34 pm
- Forum: General Rate Laws
- Topic: Enzyme saturation
- Replies: 6
- Views: 367
Re: Enzyme saturation
If an enzyme is saturated, then the reaction rate is not going to increase even if the concentration of reactant increases.
- Sun Mar 08, 2020 11:33 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Intermediate Species
- Replies: 9
- Views: 647
Re: Intermediate Species
An intermediate species is a species that is formed in the middle of the reaction but does not appear in the overall reaction equation or overall reaction rate equation.
- Sun Mar 08, 2020 11:32 pm
- Forum: General Rate Laws
- Topic: First vs Second vs Zero Order
- Replies: 7
- Views: 540
Re: First vs Second vs Zero Order
A first order reaction is one that is a straight line on the ln[a] vs time graph. A second order reaction is one that is a straight line on the 1/[a] vs time graph.
- Sun Mar 08, 2020 11:31 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Notation Layout
- Replies: 7
- Views: 386
Re: Cell Notation Layout
For a galvanic cell, the oxidation is on the left and the reduction is on the right.
- Mon Mar 02, 2020 10:30 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: test 2 topics
- Replies: 11
- Views: 701
Re: test 2 topics
Will section 6O be on the test because it covers some concepts we didn't go over in class?
- Mon Mar 02, 2020 10:29 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: gibbs free energy vs cell standard potential
- Replies: 3
- Views: 200
Re: gibbs free energy vs cell standard potential
This is because in the equation, deltaG = -nFE, the n compensates for the change in the molar quantities so E has to remain the same for deltaG to change.
- Mon Mar 02, 2020 10:28 am
- Forum: Balancing Redox Reactions
- Topic: Anode and Xathod
- Replies: 9
- Views: 500
Re: Anode and Xathod
An anode is the site of oxidation and cathode is the site of reduction.
- Mon Mar 02, 2020 10:27 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Notation Layout
- Replies: 7
- Views: 386
Re: Cell Notation Layout
Yes. Typically, you write the oxidation (anode) on the left and the reduction(cathode) on the right.
- Mon Mar 02, 2020 10:26 am
- Forum: First Order Reactions
- Topic: First Order Reaction
- Replies: 4
- Views: 359
Re: First Order Reaction
A first order reaction is characterized by the linear graph of concentration and time.
- Mon Mar 02, 2020 10:24 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Concentration in Cell Notation
- Replies: 2
- Views: 171
Re: Concentration in Cell Notation
If the question is asking you to find an unknown concentration in the cell diagram, then I would write it as part of it.
- Thu Feb 20, 2020 12:00 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: galvanic cell structure
- Replies: 8
- Views: 354
Re: galvanic cell structure
At the anode, the electrons leave the electrode and migrate to the cathode. Thus, the anode is oxidized while the cathode is reduced.
- Wed Feb 19, 2020 11:59 pm
- Forum: Balancing Redox Reactions
- Topic: Understanding Half-Reactions
- Replies: 11
- Views: 632
Re: Understanding Half-Reactions
The half-reactions represent the oxidation and reduction reactions. For a species to be reduced, it has to accept electrons from a species that has to be oxidized.
- Wed Feb 19, 2020 11:58 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Max Potential
- Replies: 5
- Views: 302
Re: Max Potential
Maximum voltage occurs right when the switch is closed, which is when there is least current flowing.
- Wed Feb 19, 2020 11:57 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Battery Dying
- Replies: 4
- Views: 296
Re: Battery Dying
The salt bridge allows the charge to be balanced on both sides, therefore it allows the charge to continue transferring.
- Wed Feb 19, 2020 11:57 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Dead Battery
- Replies: 6
- Views: 376
Re: Dead Battery
A battery goes dead when the reaction inside has reached equilibrium ( the transfer of net charge has stopped).
- Wed Feb 19, 2020 11:56 pm
- Forum: Balancing Redox Reactions
- Topic: Reduction vs. oxidation
- Replies: 29
- Views: 1072
Re: Reduction vs. oxidation
Reduced species are those that gain electrons and oxidized species are those that lose electrons.
- Wed Feb 19, 2020 11:55 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Potential difference between electrodes
- Replies: 3
- Views: 270
Re: Potential difference between electrodes
The maximum voltage occurs just when the switch is closed. This is because voltage is equal to J/Coulomb of charge and since charge is in the denominator, maximum voltage occurs at the least charge.
- Wed Feb 19, 2020 11:53 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Adding Inert Gas
- Replies: 20
- Views: 1018
Re: Adding Inert Gas
Adding an inert gas does not shift the reaction because it doesn't react with any of the reactants or products so the concentrations of each don't change.
- Wed Feb 19, 2020 11:52 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Gibbs free energy
- Replies: 9
- Views: 665
Re: Gibbs free energy
The second one is gibbs free energy measured under standard conditions. This gibbs free energy remains constant throughout the reaction .
- Wed Feb 19, 2020 11:51 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Anode and Cathode
- Replies: 6
- Views: 380
Re: Anode and Cathode
The anode is always oxidized and the cathode is always reduced, so the electron will always travel from the anode to the cathode.
- Mon Feb 10, 2020 12:08 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 4D.3
- Replies: 2
- Views: 157
Re: 4D.3
This is in a bomb calorimeter so volume is constant, so no work is done. delta U is equal to q, which is C(deltaT). C is the capacity of the bomb calorimeter and T is the temperature change given.
- Mon Feb 10, 2020 12:04 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: constant pressure system
- Replies: 2
- Views: 224
Re: constant pressure system
An open system is always constant pressure because the system is exposed to the air which is at constant pressure.
- Mon Feb 10, 2020 12:01 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: spontaneity
- Replies: 18
- Views: 646
Re: spontaneity
a reaction is spontaneous if the total entropy is positive
- Mon Feb 10, 2020 12:00 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: spontaneity
- Replies: 18
- Views: 646
Re: spontaneity
a reaction is spontaneous if the total entropy is positive
- Sun Feb 09, 2020 8:33 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: State Functions
- Replies: 5
- Views: 494
Re: State Functions
The acronym is P D TV HUGS. When your under pressure and depressed, you should watch TV and gets hugs. P = Pressure, D = density, T = temperature, V = volume, H = enthalpy, U = internal E, G = gibbs free energy, and S = entropy. Heat capacity is also a state function.
- Mon Jan 27, 2020 8:58 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Chemical Equilibria
- Replies: 4
- Views: 248
Re: Chemical Equilibria
When a reaction has reached equilibrium, the rate at which products are formed is equal to the rate at which reactants are formed. The concentrations of reactants and products remain constant.
- Mon Jan 27, 2020 8:55 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Negative delta H
- Replies: 2
- Views: 95
Re: Negative delta H
In a reaction, you have both the breaking of bonds and forming of bonds. Therefore, there are energy requirements and energy release involved in a reaction. Just depends on whether the requirement out-weights the release or not.
- Mon Jan 27, 2020 8:53 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: q and deltaH
- Replies: 3
- Views: 90
Re: q and deltaH
delta H is the heat measured under constant pressure.
- Mon Jan 27, 2020 8:53 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Ka and Kb
- Replies: 10
- Views: 304
Re: Ka and Kb
If Ka is less than 10-3, then it is a weak acid. Greater than 10^3 would make it a strong acid.
- Mon Jan 27, 2020 8:51 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Specific Heat and Molar Heat Capacity
- Replies: 4
- Views: 194
Re: Specific Heat and Molar Heat Capacity
Heat capacity is an extensive property while specific heat capacity is an intensive property. Intensive properties are more important to us.
- Mon Jan 27, 2020 8:50 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Stirrer in Calorimeter?
- Replies: 3
- Views: 373
Re: Stirrer in Calorimeter?
The stirrer also helps to homogenize the solution so that the change in temperature is distributed evenly.
- Mon Jan 27, 2020 8:49 pm
- Forum: Phase Changes & Related Calculations
- Topic: Enthalpy Intensive or Extensive
- Replies: 4
- Views: 2762
Re: Enthalpy Intensive or Extensive
Enthalpy is an extensive property. Another extensive property is heat capacity. Specific heat capacity, however, is an intensive property.
- Mon Jan 27, 2020 8:48 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Calorimeter
- Replies: 7
- Views: 483
Re: Calorimeter
A calorimeter is an instrument used to calculate the change in Temperature caused by a reaction and using this change to calculate the enthalpy of reaction.
- Mon Jan 27, 2020 8:46 pm
- Forum: Phase Changes & Related Calculations
- Topic: Enthalpy of sublimation?
- Replies: 8
- Views: 1334
Re: Enthalpy of sublimation?
The enthalpy of sublimation is simply the sum of the heat of fusion and the heat of vaporization.
- Mon Jan 20, 2020 6:09 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: q vs k
- Replies: 62
- Views: 2320
Re: q vs k
Q value is calculated when you don't know whether the reaction is at equilibrium or not. If Q equals K, then the reaction is at equilibrium.
- Mon Jan 20, 2020 6:09 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Endothermic vs Exothermic
- Replies: 7
- Views: 290
Re: Endothermic vs Exothermic
An exothermic reaction will have a delta H value that is negative and an endothermic reaction will have a delta H value that is positive.
- Mon Jan 20, 2020 6:03 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: definition of a buffer
- Replies: 8
- Views: 382
Re: definition of a buffer
A buffer is a solution that contains both conjugates. In the ICE table, therefore, the starting concentration for the conjugate acid/base is not 0.
- Mon Jan 20, 2020 6:02 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Writing K Expression
- Replies: 6
- Views: 195
Re: Writing K Expression
Yes, H20 is included in the K equation when it is a gas.
- Mon Jan 20, 2020 6:01 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ATP hydrolysis [ENDORSED]
- Replies: 3
- Views: 96
Re: ATP hydrolysis [ENDORSED]
Because ATP hydrolysis is exergonic, so the products have less energy than the reactants. Thus, the products are more stable than the reactants.
- Mon Jan 20, 2020 5:57 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE table and X
- Replies: 6
- Views: 265
Re: ICE table and X
You eliminate x from the denominator when K is less than 0.001. This is because when K is this small, the change (x) will be less than 5% of the initial concentration.
- Sun Jan 12, 2020 9:32 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Q>K
- Replies: 9
- Views: 239
Re: Q>K
Q is greater than K when there more products than the equilibrium concentration of products.
- Sun Jan 12, 2020 9:31 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Calculating Q
- Replies: 16
- Views: 656
Re: Calculating Q
Calculating Q is the same as calculating K.
- Sun Jan 12, 2020 9:29 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Response of Equilibria to Change
- Replies: 6
- Views: 126
Re: Response of Equilibria to Change
If stress is put on a system, then the reaction shifts in the direction that minimizes that stress.
- Sun Jan 12, 2020 9:28 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K and Q
- Replies: 10
- Views: 248
Re: K and Q
K and Q are different because K represents the reaction at equilibrium whereas Q represents the reaction at a point other than at equilibrium.
- Sun Jan 12, 2020 9:26 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Solids and Liquids
- Replies: 6
- Views: 116
Re: Solids and Liquids
Solids are not used because you cannot measure the concentration of solids. Liquids are not used because pure liquids are too dilute to affect the K.
- Sat Dec 07, 2019 11:17 pm
- Forum: Calculating the pH of Salt Solutions
- Topic: weak acid/base and pH
- Replies: 9
- Views: 646
Re: weak acid/base and pH
A weak base will not raise the pH as much as a strong base would and that also goes for weak acids as they are incompletely protonated/deprotonized.
- Sat Dec 07, 2019 11:15 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: bond angles
- Replies: 16
- Views: 1095
Re: bond angles
Bond angles will be less than the ideal structure due to lone pair and bond pair repulsion and/or lone-pair lone-pair repulsions.
- Sat Dec 07, 2019 11:13 pm
- Forum: Air Pollution & Acid Rain
- Topic: dirty/clean coal
- Replies: 6
- Views: 400
Re: dirty/clean coal
Dirty coal has more Sulfur in it while clean coal has less sulfur content and thus more Carbon content.
- Sat Dec 07, 2019 11:13 pm
- Forum: Biological Examples
- Topic: Cisplatin
- Replies: 5
- Views: 504
Re: Cisplatin
Cis can form two bonds because the Chlorines are on the same side, while in trans they are opposite of each other.
- Sat Dec 07, 2019 11:12 pm
- Forum: Air Pollution & Acid Rain
- Topic: Acid Rain
- Replies: 24
- Views: 3710
Re: Acid Rain
I don't think we need to know its impact on the environment. We just need to know the chemical equations associated with it and that the primary acid in acid rain is carbonic acid.
- Sun Dec 01, 2019 11:31 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Relative Acidity
- Replies: 1
- Views: 57
Re: Relative Acidity
Relative strength of an acid can be calculated using the Ka value of the acid, assuming the acid is a weak acid. Ka = [H+][A-]/[HA]. The higher the Ka value, the stronger the acid.
- Sun Dec 01, 2019 11:28 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: pOH
- Replies: 3
- Views: 101
Re: pOH
[OH-][H+] = 1x10^14, which is equal to Kw. If we take the -log of each side, we get pOH + pH = 14. Knowing the pOH will allow you to calculate the pH of the solution.
- Sun Dec 01, 2019 11:26 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Acid and water
- Replies: 2
- Views: 112
Re: Acid and water
It is more accurate to use H3O+ in place of H+ because the acid will donate its proton to the water molecule to form H3O+. Calculating pH is the same if you take H3O+ in place of H+.
- Sun Dec 01, 2019 11:23 pm
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: pKa and electronegativity
- Replies: 2
- Views: 136
Re: pKa and electronegativity
In binary acids H-A, the greater the electron affinity and thus the electronegativity of the A element, the more polarizing the molecule and thus, the Hydrogen is more easily lost to a proton acceptor and thus, its Ka value will be greater and pKa will be smaller compared to that of a binary acid in...
- Sun Dec 01, 2019 11:20 pm
- Forum: Lewis Acids & Bases
- Topic: Difference between Lewis and Bronsted
- Replies: 4
- Views: 270
Re: Difference between Lewis and Bronsted
Lewis acids accept electron pairs and Lewis bases donate electron pairs while Bronsted acids donate protons and Bronsted bases accept protons. Lewis acids includes the proton while Bronsted only considers compounds as acidic if they supply protons.
- Sun Dec 01, 2019 11:18 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Acids Vs. Bases
- Replies: 11
- Views: 817
Re: Acids Vs. Bases
Acid and Base classification differs depending on whether you are discussing Arrhenius, Bronsted, or Lewis acids and bases. Arrhenius acids form H+ ions in water, while bases form OH- ions in water. Bronsted acids donate protons while Bronsted bases accept protons. Lewis acids accept electron pairs ...
- Sun Nov 24, 2019 11:47 pm
- Forum: Hybridization
- Topic: Sigma and Pi Bonds
- Replies: 21
- Views: 917
Re: Sigma and Pi Bonds
All single bonds are sigma bonds. In double or triple bonds, there is one sigma bond and the rest are pi.
- Sun Nov 24, 2019 11:43 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Bond Order
- Replies: 14
- Views: 945
Re: Bond Order
If a bond order is zero, that means that the molecule is too unstable and it will not exist.
- Sun Nov 24, 2019 11:31 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Cis vs Trans
- Replies: 22
- Views: 1549
Re: Cis vs Trans
cis indicates that the functional groups are on the same side of the carbon chain while trans conveys that functional groups are on opposing sides of the carbon chain
- Sun Nov 24, 2019 11:26 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 7
- Views: 453
Re: Bond Angles
If the atoms bonded to the central atom are not the same, the size and electron distribution around the atoms will differ which will affect the distribution of the electrons on the other atoms, which will affect the bond angle.
- Sun Nov 24, 2019 11:24 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Hydrogen Bonding
- Replies: 2
- Views: 142
Re: Hydrogen Bonding
A lone pair is a potential site for hydrogen bonding. Hydrogen bonding can also be possible when hydrogen is near a nitrogen, oxygen, or fluorine atom.
- Sun Nov 17, 2019 9:53 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 7
- Views: 403
Re: Bond Angles
Lone pair - lone pair repulsion is stronger than lone-pair bond pair which is stronger than bond pair-bond pair, regardless of whether it involves a cation, anion, or molecule.
- Sun Nov 17, 2019 9:51 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: vsepr angles
- Replies: 10
- Views: 402
Re: vsepr angles
You should memorize the different orientations and their bond angles as it will be useful for the upcoming test.
- Sun Nov 17, 2019 9:51 pm
- Forum: Dipole Moments
- Topic: Effects for boiling point
- Replies: 5
- Views: 309
Re: Effects for boiling point
Boiling point increases when the strength of the intermolecular force increases. For instance, molecules that have induced-dipole attraction have a lower boiling point that molecules that interact through ionic interactions.
- Sun Nov 17, 2019 9:49 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: covalent forces
- Replies: 1
- Views: 120
Re: covalent forces
A non-covalent interaction is different from covalent because it does not involve the sharing of electrons, but instead has more dispersed variations of electromagnetic interactions between or within molecules.
- Sun Nov 17, 2019 9:48 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: intermolecular forces
- Replies: 2
- Views: 127
Re: intermolecular forces
induced dipole-dipole are not permanent forces. They are temporary dipoles that have been induced by a neighboring molecule. Also, most intermolecular forces are not permanent.
- Sat Nov 09, 2019 11:34 pm
- Forum: Sigma & Pi Bonds
- Topic: One Sigma One Pi
- Replies: 3
- Views: 216
Re: One Sigma One Pi
Two sigma bonds are not possible because the orbitals overlap end-to-end in a sigma bond. In order to form another bond to share more electrons, it is only possible for their orbitals to overlap side-to-side to form a pi bond.
- Sat Nov 09, 2019 11:14 pm
- Forum: Hybridization
- Topic: Pi vs Sigma Bonds
- Replies: 4
- Views: 281
Re: Pi vs Sigma Bonds
Pi bonds are weaker than sigma bonds because the of the parallel orbital paths which mean less overlap between the p-orbitals. Pi bonds happen when two atomic orbitals are in contact through two areas of overlap. Pi bonds are also more spread out than sigma bonds.
- Sat Nov 09, 2019 11:10 pm
- Forum: Ionic & Covalent Bonds
- Topic: Comparing Strengths of Ionic & Covalent Bonds
- Replies: 2
- Views: 149
Re: Comparing Strengths of Ionic & Covalent Bonds
When aqueous environment, covalent bond are stronger than ionic bonds because compounds held together by ionic bonds tend to dissolve in water and dissociate into the individual ions whereas the molecules in molecular compounds do not break up when in water.
- Sat Nov 09, 2019 11:03 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angle
- Replies: 2
- Views: 82
Re: Bond Angle
The lone pairs are delocalized whereas the electrons in a bond are not free to move as much. Therefore, the repulsions between the electrons in lone pairs can distort the electron cloud.
- Sat Nov 09, 2019 10:50 pm
- Forum: Electronegativity
- Topic: Ionization Energy
- Replies: 3
- Views: 147
Re: Ionization Energy
Nitrogen also has a lower IE because it has half-filled p subshell which is more stable than the 4 electron configuration in the p orbital of oxygen.
- Sun Nov 03, 2019 9:51 pm
- Forum: Properties of Electrons
- Topic: Electrons
- Replies: 1
- Views: 203
Re: Electrons
In a many electron system, the orbitals within a shell differ in their energies. This difference is attributed to electron-electron repulsions within the orbitals. This is different from a one electron system, in which the orbitals within a shell are degenerate (are of the same energies).
- Sun Nov 03, 2019 9:49 pm
- Forum: *Shrodinger Equation
- Topic: Schrodinger's Equation
- Replies: 1
- Views: 213
Re: Schrodinger's Equation
Electrons have wave-particle duality. Schrodinger equation is used to represent the wave-like characteristic of electrons. The square of the wave function represents the probability density of finding an electron in a particular space.
- Sun Nov 03, 2019 9:47 pm
- Forum: Octet Exceptions
- Topic: d-Orbitals
- Replies: 2
- Views: 79
Re: d-Orbitals
Usually you can tell if you need the incomplete octet when the number of total electrons doesn't equal the total number of electrons in the structure and you cant accommodate with more bonds.
- Sun Nov 03, 2019 9:43 pm
- Forum: Bond Lengths & Energies
- Topic: Bond Strength and Electronegativity
- Replies: 3
- Views: 235
Re: Bond Strength and Electronegativity
What is the trend of electronegativity in terms of the periodic table? Does electronegativity increase as you go towards the right of the periodic table? The trend for electronegativity is that it increases diagonally from bottom left to the top right. Flourine, therefore, is the most electronegati...
- Sun Nov 03, 2019 9:41 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: formal charge
- Replies: 5
- Views: 176
Re: formal charge
Formal charge is calculated by subtracting the number of bonds plus the number of free electrons from the number of valence electrons of that atom. The sum of the number of bonds plus the number of free electrons can be thought of as the sum of the number of sticks (bonds) and dots (electrons).
- Sun Oct 27, 2019 12:13 am
- Forum: Quantum Numbers and The H-Atom
- Topic: Quantum Numbers
- Replies: 7
- Views: 208
Re: Quantum Numbers
Electron spins affect an electron's behavior because it prevents two electrons with parallel spins from occupying the same orbital. The configuration is most stable when electrons are paired with electrons with opposite spins.
- Sun Oct 27, 2019 12:10 am
- Forum: Trends in The Periodic Table
- Topic: Angstroms and Atomic Radii
- Replies: 2
- Views: 63
Re: Angstroms and Atomic Radii
The atomic radius is measured by halving the inter-nuclear distance between two like atoms. This is what the Angstrom represents.
- Sun Oct 27, 2019 12:08 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Lowering Formal Charge
- Replies: 6
- Views: 646
Re: Lowering Formal Charge
The arrangement that allows for the lowest formal charge is the one that matches closest to the true structure. Also, it is important to remember that the atom with the lower electron affinity should not get the most negative formal charge.
- Sun Oct 27, 2019 12:05 am
- Forum: Trends in The Periodic Table
- Topic: Aufbau Principle
- Replies: 11
- Views: 544
Re: Aufbau Principle
Can someone explain how to set this up so that you can get to the electron configuration. I understand that you want to fill the shells so that they become more stable and how to put in the spin state but what is the order that you fill in the shells? You fill the shells in order of increasing ener...
- Sun Oct 27, 2019 12:00 am
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Same spin
- Replies: 10
- Views: 469
Re: Same spin
Aprice_1J wrote:When would you see them have parallel spins? If they are more stable with different spins, what would constitute them having the same spin?
Electrons with the same spin cannot occupy the same orbital. Electrons singly occupy the different orbitals with parallel spins (Hund's Rule).
- Wed Oct 16, 2019 10:02 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Stern and Gerlach
- Replies: 5
- Views: 236
Re: Stern and Gerlach
The difference in spin only shows up in the presence of a magnetic field. In the absence of magnetic field, the electron spins have the same energy, however, this is not the case when the atom beam of silver ions passed through a magnetic field in the experiment.
- Wed Oct 16, 2019 10:01 pm
- Forum: *Shrodinger Equation
- Topic: Hamiltonian
- Replies: 1
- Views: 107
Re: Hamiltonian
If a wave equation represents electrons, a change in the wave function will give the energy associated with the wave function. The double derivative of the wave function allows us to return to the original equation. For example, when we take the derivative of sinx, we get cosx, and when we take the ...
- Wed Oct 16, 2019 9:55 pm
- Forum: Properties of Electrons
- Topic: The wave property of electrons [ENDORSED]
- Replies: 2
- Views: 113
Re: The wave property of electrons [ENDORSED]
If electrons only acted as particles, there would be no diffraction pattern. The electrons would have been detected in one spot as opposed to more than one.
- Wed Oct 16, 2019 9:50 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Subshell and orbital clarification
- Replies: 1
- Views: 64
Re: Subshell and orbital clarification
The number of orbitals are usually found using the magnetic quantum number, m subscript l. For example, the quantum number l = 1 would have ml equal to -1, 0, 1 which corresponds to 3 p orbitals. The p is found based on the value of l. A value of 0 corresponds to s orbital, 1 to p orbital, 2 to d or...
- Wed Oct 16, 2019 9:45 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Schrodinger's Wave Equation
- Replies: 2
- Views: 65
Re: Schrodinger's Wave Equation
It applies to one electron systems only because for one electron systems, the different energy levels are degenerate, or equal in energy. However, for multi-electron systems, this is not true.
- Sun Oct 13, 2019 6:53 pm
- Forum: Properties of Light
- Topic: Visualizing wave-particle duality
- Replies: 3
- Views: 146
Re: Visualizing wave-particle duality
The wavelength of light is different from the wavelength of a photon/electron. The equation for light is c = wavelength x frequency, whereas, the equation for wavelength of an electron is wavelength = h (Planck's constant)/p (momentum).
- Sun Oct 13, 2019 6:50 pm
- Forum: Properties of Light
- Topic: 'light intensity'
- Replies: 8
- Views: 215
Re: 'light intensity'
Black body refers to anything that absorbs all forms of electromagnetic radiation, regardless of frequency.
- Sun Oct 13, 2019 6:48 pm
- Forum: Properties of Light
- Topic: Quanta- clear up comparison
- Replies: 3
- Views: 162
Re: Quanta- clear up comparison
The example relates to quanta because in the quantum world, energy is assumed to be in quantized, or discreet amounts rather than being continuous. On the surface, the water from the bucket looks like it is flowing in one continuous motion. However, when you are on the molecular level, water is comi...
- Sun Oct 13, 2019 6:45 pm
- Forum: Properties of Light
- Topic: P.E Experiment
- Replies: 3
- Views: 186
Re: P.E Experiment
When an electron moves from a higher energy level to a lower energy level, it emits or releases energy. The release of energy is associated with a more stable state. Transitioning from n=4 to n=2 allows the electron to achieve a more stable state, and thus, it emits energy.
- Sun Oct 13, 2019 6:42 pm
- Forum: Properties of Light
- Topic: Wave vs particle properties
- Replies: 4
- Views: 379
Re: Wave vs particle properties
It is also important to remember that equations for electromagnetic radiation (waves) cannot be directly applied to equations for measuring wavelength associated with an electron. For example, the equation: c = lamda x frequency cannot be used to solve for the electron's wavelength. There is a separ...
- Wed Oct 02, 2019 5:18 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Tips on how to write a formula out from the name
- Replies: 9
- Views: 656
Re: Tips on how to write a formula out from the name
There's a list of strong acids and bases in the textbook which would come in handy for some of the problems, so I suggest memorizing them. Learning these would also help with understanding the nomenclature pattern of acids/bases and the ions involved.
- Wed Oct 02, 2019 5:11 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: General Rounding Question
- Replies: 9
- Views: 308
Re: General Rounding Question
Try to avoid rounding until the very end when you have to give the answer with the correct number of significant figures, which is the least number of significant figures among the numbers given in the question.
- Wed Oct 02, 2019 5:07 pm
- Forum: Limiting Reactant Calculations
- Topic: Other Way to Find the Limiting Reactant [ENDORSED]
- Replies: 3
- Views: 154
Re: Other Way to Find the Limiting Reactant [ENDORSED]
To find the limiting reactant, I find it helpful to calculate the number of moles of other reactants required for each reactant and then comparing that value to the number of moles that actually exist for each reactant.
- Wed Oct 02, 2019 12:53 am
- Forum: SI Units, Unit Conversions
- Topic: Writing chemical equations
- Replies: 2
- Views: 149
Re: Writing chemical equations
Chemical equations can be divided up into combination, decomposition, single displacement, double displacement, combustion, and redox reactions. Combination involves two or more reactants that form one product and decomposition is the reverse of that. In single displacement, the more active element ...